Chapter 8.1, Problem 2PP

Interpretation Introduction

Interpretation: The Lewis dot structure of H₂ S needs to be drawn.

Concept introduction: Lewis structure is shown by each atom in the molecule using the chemical symbol with the electron. The bond is formed by sharing of electron between the atoms and excess electrons are shown as lone pairs.

Answer to Problem 2PP

After sharing the electron between $\text{Hydrogen}\left(\text{H}\right)$ and $\text{Sulphur}\left(\text{S}\right)$ , the valence shells configuration can be achieved and a stable structure is formed.

Explanation of Solution

Lewis structure of ${\text{H}}_{\text{2}}\text{S}$ :

First write the electron configuration for $\text{Hydrogen}\left(\text{H}\right)$ and $\text{Sulphur}\left(\text{S}\right)$ :

$\text{H}\to 1{\text{s}}^1$

$\text{S}\to 1{\text{s}}^{2}2{\text{s}}^{2}2{\text{p}}^{6}3{\text{s}}^{2}3{\text{p}}^4$

$\text{Hydrogen}\left(\text{H}\right)$ and $\text{Sulphur}\left(\text{S}\right)$ has $1$ electron and $6$ electrons in their outermost shell respectively.

For the valence shell configuration or stable structure formation, $\text{hydrogen}$ requires $1$ electron and $\text{sulphur}$ requires $2$ electrons respectively to achieve octet configuration.

After sharing the electron between $\text{Hydrogen}\left(\text{H}\right)$ and $\text{Sulphur}\left(\text{S}\right)$ , the stable valence shell configuration and stable structure can be obtained.

Conclusion

The valence shell configuration can be achieved by sharing the electrons.